Calculate the concentration of silver in each sample. Are there any problems? How will you address each of the identified problems? Standards Absorbance Ag (ppb) 0.00 0.000 2.00 0.013 10.0 0.076 20.0 0.162 30.0 0.245 50.0 0.405 75.0 0.598 100.0 0.748 Samples Absorbance 08002 0.079 08003 0.058 08004 0.129 08005 0.082 08006 0.797 08007 0.063 08008 0.009 08009 0.028 08010 0.136
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- Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choices1. A student performed this experiment and obtained the following concentration values: 0.02813 M, 0.02802, and 0.02788 M a. what is the mean concentration? b. what is the standard deviation of these results? 3. how would the following errors affect the concentration of Cl- obtained in question 2b? give your reasoning in each case. a. the student read the molarity of AgNo3 as 0.02104M instead of 0.02014M b. the student was past the endpoint of titration when he took the final buret reading.4. A new procedure for the determination of sulfur in coal was tested on a standard coal sample with a certified value of 2.14% sulfur by mass. The new procedure gave results of 2.11%, 2.07%, 2.04%, 2.06%, and 2.16% for five separate determinations. a) Does the new procedure give the correct result at the 95% confidence level? b) Does the new procedure give the correct result at the 90% confidence level?
- The molarity of a solution is determined by four separate titrations or replicates, where the obtained data was 0.4120, 0.4920, 0.3920, and 0.4320 M. Calculate the standard error of the mean for the above data. O 0.00185 O 0.02160 O 0.43200 O 0.04320 O 0.01080Name: Date: Section: Data Report Sheet: Analysis of an Unknown Chloride Unknown # -2 Molarity of Standard Ag(NO), 5.2167x10 M Trial I Trial II Trial III Mass of Unknown 0.237 o. 232 g g Initial Burette Reading 0.00 mL 7.90 mL mL Final Burette Reading 31.00 mL 42.00 mL mL Vol. Ag(NO3) Added 31.00 mL 34.10 mL mL Moles Ag(NO,) 1.617177y10 mol. 1,7789 v10 mol. Moles CI 1.617177x103mdl. Mass Cl 0.05741 8 0g 24.22 % 27.22% Cl in Unknown Average % Cl in unknown 25.720%. In C.AJ = - kt.tln [A.o]. t¹/₂ = 0.693 K In = KE •1• [A]o⋅=⋅· 100 ·/. [A] + = left . CAJO. CAJE In. [100] [s] t =.kt K= 0.693 t¼½₂ CAJO t = |n² Ch t = ln [AG] ·K CAJO K= In [At]. t Formulas Problem: Na-24 has a half life of 15 hours. How much of a 20.09. ·Sample would remain after decaying for 60 hours? Plz explain step by step. using the formulas..
- Based on this student data, calculate the average molarity of the NaOH solution. Standard: KHP = potassium hydrogen phthalate, MM 204.4 g/mol Student Data Trial 1 E KHP mL initial: NaOH mL final: NaOH 2.02 0.57 19.25 Trial 2 2.05 19.25 39.80 Trial 3 1.99 1.65 20.75only need help with "e" 1. Use the following data table and steps a-d below to calculate the concentration of the zinc carbonate. The mass of the filter paper alone (no ZnCO3) was 1.3457 g. The Zn(NO3)2 solution (10.00 mL) was mixed with 15.00 mL of the 1.00 M Na2CO3. a. Calculate the mass of zinc carbonate formed. 0.8939 b. How many moles of zinc carbonate formed? 0.00715 c. Calculate the moles of zinc in the zinc nitrate solution used. 0.00175 d. Calculate the concentration of the zinc in the zinc nitrate solution. 0.715 M e. Confirm whether sodium carbonate was in excess. Using the concentration of the sodium carbonate solution used, determine how many moles were used and confirm it was the excess reagentA solution is made by the following steps. 1. 90.0 mg ± 0.2 mg of dye with molar mass 685.79 g/mol ± 0.02 g/mol is dissolved in a 100.00 mL ± 0.05 mL volumetric flask with water to make solution #1. 2. 25.00 mL of solution 1 is added 100.00 mL ± 0.05 mL volumetric flask with water to make solution #2. 3. 25.00 mL of solution 2 is added 100.00 mL ± 0.05 mL volumetric flask with water to make solution #3. A.) If you have available a 5.00 mL ± 0.01 mL, 10.00 mL ± 0.05 mL, and 25.00 mL± 0.15 mL. Describe how to use the pipettes and the directions above to make the most precise solution #3. Explain why this is the most precise method. B.) Determine the concentration ± absolute error of solution #3 in molarity. Explain the calculations you needed to do. C.) Using Beer's law (10% error), solution #3 is found to be 2.0 ✕ 10-5 M. Was solution #3 likely made within the expected error. Explain.
- 6.20 mL of tap water sample is taken in a conical flask and 1 mL of pH 10 buffer and 3 drops of iochrome black-T indicator are added and when titrated with 0.001 M EDTA solution, 16 mL EDTA is spent, so the hardness of the water is determined by French Hardness and German Hardness Calculate in terms.A sample contains FeS2. At the end of its gravimetric determination, BaSO4 is weighed and the percentage of Fe is being searched for. What is an expression for the gravimetric factor in this determination? (The formulas represent the formula weights) a) FeS2 / BaSO4 b) Fe /2 BaSO4 c) 2 Fe / BaSO4 d) FeS2 / 2 BaSO4 e) 2 FeS2 / BaSO4Foreattt part of iTIS qtestfoni; tonsider FOHOWIHg Btetat: You need to make a stock solution of Ca( C2H3O2 )2 with a concentration of 6.50 M. You have a 850.0 mL volumetric flask available to make this stock solution in. You are then tasked with using this stock solution to prepare a sample for use in an experiment. The experimental sample should have a final volume of 15.0 mL and a concentration of 0.350 M Ca(C2H3O2)2. a) What is the molar mass of Ca(C2H3O2)2? b) How many moles of the solute would be needed to create the stock solution using the volumetric flask available? c) How many grams of the solute should be added to the volumetric flask to create the stock solution? d) What volume, in mL, of the stock solution should be used to prepare the experimental solution through dilution? US 目 M